Use the van der Waals equation to calculate the

pressureexerted by 1.000 mol of Cl2 in 22.41 L at 273 K.

The van der Waals constants for Cl2 are: a =

6.49L2 atm/mol2 and b =.0562 L/mol.

P = 0.9885 atm

Explanation:

Van der Waals eq:

P = (RT / (Vm - b)) - (a/Vm²)

∴ Vm = 22.41 L / 1.000 mol = 22.41 L/mol

∴ R = 0.082 atm. L/Kmol

∴ T = 273 K

∴ a Cl2 = 6.49 L²atm/mol²

∴ b Cl2 = 0.0562 L/mol

⇒ P = ((0.082 atmL/Kmol) (273 K) / (22.41 L/mol - 0.0562 L/mol)) - ((6.49 L²atm/mol²) / (22.41 L/mol) ²)

⇒ P = (1.0014 atm) - (0.013 atm)

⇒ P = 0.9885 atm